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A mixture of two gases has a total pressure of 5.7 ATM If one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
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What is Daltons law on partial pressure?
Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture. Each gas in a mixture exerts a pressure that is independent of the other gases present.
What does Dalton's law of partial pressures?
The total pressure of a gas mixture is the sum of the individual pressures.
If a mixture of two gases has a total pressure of 5.7 ATM. If one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
What happens to the partial pressure of oxygen in the air if the air temp increases?
When the air temperature increases, the partial pressure of oxygen remains the same in the air. This is because the partial pressure of a gas in a mixture is determined by its concentration and is independent of the temperature, assuming the volume and moles of other gases remain constant.
Why is Dalton's Law a limiting law?
A limiting law is such a law that is strictly true in a certain limit.Now, Dalton's law states that: The pressure exerted by a mixture of gases is the sum of the pressures that each one would exert if it occupied the container alone.The law that the sum of the partial pressures equals the total pressure is true for real and perfect gases.Whereas, the identification of partial pressure with pressure that a gas would exert on its own is only valid for a perfect gas.So now we see that Dalton's law is only valid for perfect gases, hence it is a limiting law.Hope that helps.
A mixture of two gases has a total pressure of 5.7 if one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
A mixture of two gases has a total pressure of 5.7 ATM if one has has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
A mixture of two gases has a total pressure a 5.7 ATM if one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
A Mixture Of Two Gases Has A Total Pressure Of 5.7 Atm. If One Gas Has A Partial Pressure Of 4.1 Atm What Is The Partial Pressure Of The Other Gas?
1.6 ATM
What is Daltons law on partial pressure?
Dalton's law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture. Each gas in a mixture exerts a pressure that is independent of the other gases present.
What does Dalton's law of partial pressures?
The total pressure of a gas mixture is the sum of the individual pressures.
If a mixture of two gases has a total pressure of 5.7 ATM. If one gas has a partial pressure of 4.1 ATM what is the partial pressure of the other gas?
1.6 ATM
The difference between vapor pressure of a pure solvent and its partial pressure?
vapor pressure of a pure solvent is the pressure needed for the gas to escape the pure solvent in vapor form. its partial pressure in this case will be the pressure of that escaped vapour (in the mixture of air). in simpler terms vapor pressure describes a single condensable system (just the vapor of the solvent and the liquid state of the solvent) while its partial pressure describes the multicomponent system (air). they are essentially the same thing describing different systems
What happens to the partial pressure of oxygen in the air if the air temp increases?
When the air temperature increases, the partial pressure of oxygen remains the same in the air. This is because the partial pressure of a gas in a mixture is determined by its concentration and is independent of the temperature, assuming the volume and moles of other gases remain constant.
Why is Dalton's Law a limiting law?
A limiting law is such a law that is strictly true in a certain limit.Now, Dalton's law states that: The pressure exerted by a mixture of gases is the sum of the pressures that each one would exert if it occupied the container alone.The law that the sum of the partial pressures equals the total pressure is true for real and perfect gases.Whereas, the identification of partial pressure with pressure that a gas would exert on its own is only valid for a perfect gas.So now we see that Dalton's law is only valid for perfect gases, hence it is a limiting law.Hope that helps.
A sample of dry air contains 210 mL of oxygen 780 mL of nitrogen and 10.0 mL of all other gases What is the pressure in mm of Hg due to the nitrogen if the total pressure was 1000.0 mm?
Dalton says: "The partial pressure of a (non-condensing) gas in the mixture is proportional to its concentration." Since your total pressure is 1000 mmHg and the volumes all total to 1000 mL, you don't even need to take your shoes off to do the math.The nitrogen's volume is 780 ml of the total 1000 ml so its partial pressure is 780 mmHg of the total 1000 mmHg.
What is the air-gas mixture?
It is a mixture of air with one or more other gases.
